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Chapter 8: Q9 E (page 446)

Why is the concept of hybridization required in valence bond theory?

Short Answer

Expert verified

Hybridization is necessary to determine the molecular geometry of complex.

Step by step solution

01

Definition of Concept

Hybridization occurs when two or more different pure orbitals with comparable energy are mixed together to produce an equivalent amount of impure orbitals with equal energy and definite geometry, which are referred to as hybrid orbitals.

02

Explain why is the concept of hybridization required in valence bond theory

Hybridization: Hybrid orbitals are created when two or more different pure orbitals with comparable energy are mixed together to produce an equivalent amount of impure orbitals with equal energy and definite geometry. This phenomenon is known as hybridization. It uses the valence bond theory of orbitals to help determine molecular geometry.

Therefore, the molecular geometry of complexes must be determined through hybridization..

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Most popular questions from this chapter

Draw the Lewis structures for \({\rm{C}}{{\rm{O}}_{\rm{2}}}\)and\({\rm{CO}}\), and predict the number of \({\rm{\sigma }}\) and \({\rm{\pi }}\) bonds for each molecule.

(a) \({\rm{C}}{{\rm{O}}_{\rm{2}}}\)

(b) \({\rm{CO}}\)

Sketch the distribution of electron density in the bonding and antibonding molecular orbitals formed from two S orbitals and from two P orbitals.

Write Lewis structures for \({\rm{N}}{{\rm{F}}_{\rm{3}}}\) and \({\rm{P}}{{\rm{F}}_{\rm{5}}}\). On the basis of hybrid orbitals, explain the fact that \({\rm{N}}{{\rm{F}}_{\rm{3}}}\), \({\rm{P}}{{\rm{F}}_{\rm{3}}}\), and \({\rm{P}}{{\rm{F}}_{\rm{5}}}\) are stable molecules, but \({\rm{N}}{{\rm{F}}_{\rm{5}}}\) does not exist.

What charge would be needed on \({{\rm{F}}_{\rm{2}}}\) to generate an ion with a bond order of \({\rm{2}}\)?

The bond energy of a C–C single bond averages \({\rm{347 kJ mo}}{{\rm{l}}^{{\rm{ - 1}}}}\); that of a

C ≡ C triple bond averages \({\rm{839 kJ mo}}{{\rm{l}}^{{\rm{ - 1}}}}\). Explain why the triple bond is not three times as strong as a single bond.
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